Synthesis, Characterization and Catalytic Activity of ... - E-journal UNDIP

Available online at BCREC Website: http://bcrec.undip.ac.id Bulletin of Chemical Reaction Engineering & Catalysis, 10 (2), 2015, 169-174 Research Article

Synthesis, Characterization and Catalytic Activity of Cu/Cu2O Nanoparticles Prepared in Aqueous Medium Sayed M. Badawy1, 2*, R.A. El-Khashab1, 2, A.A. Nayl1, 3 1

Chemistry Department, Faculty of Science, Aljouf University, Sakaka, Kingdom of Saudi Arabia 2 National Center for Clinical and Environmental Toxicology, Faculty of Medicine, Cairo University, Cairo, Egypt 3 Hot Laboratories Centre, Atomic Energy Authority, Cairo, P.O.13759, Egypt Received: 6th January 2015; Revised: 14th March 2015; Accepted: 15th March 2015 Abstract

Copper/Copper oxide (Cu/Cu2O) nanoparticles were synthesized by modified chemical reduction method in an aqueous medium using hydrazine as reducing agent and copper sulfate pentahydrate as precursor. The Cu/Cu2O nanoparticles were characterized by X-ray Diffraction (XRD), Energy Dispersive X-ray Fluorescence (EDXRF), Scanning Electron Microscope (SEM), and Transmission Electron Microscope (TEM). The analysis revealed the pattern of face-centered cubic (fcc) crystal structure of copper Cu metal and cubic cuprites structure for Cu 2O. The SEM result showed monodispersed and agglomerated particles with two micron sizes of about 180 nm and 800 nm, respectively. The TEM result showed few single crystal particles of face-centered cubic structures with average particle size about 11-14 nm. The catalytic activity of Cu/Cu2O nanoparticles for the decomposition of hydrogen peroxide was investigated and compared with manganese oxide MnO 2. The results showed that the second-order equation provides the best correlation for the catalytic decomposition of H 2O2 on Cu/Cu2O. The catalytic activity of hydrogen peroxide by Cu/Cu2O is less than the catalytic activity of MnO 2 due to the presence of copper metal Cu with cuprous oxide Cu 2O. © 2015 BCREC UNDIP. All rights reserved. Keywords: Cu/Cu2O Nanoparticles; Copper/Copper oxide; Nanoparticles; hydrogen peroxide How to Cite: Badawy, S.M., El-Khashab, R.A., Nayl, A.A. (2015). Synthesis, Characterization and Catalytic Activity of Cu/Cu2O Nanoparticles Prepared in Aqueous Medium. Bulletin of Chemical Reaction Engineering & Catalysis, 10 (2): 169-174. (doi:10.9767/bcrec.10.2.7984.169-174) Permalink/DOI: http://dx.doi.org/10.9767/bcrec.10.2.7984.169-174

1. Introduction Nano-materials involved transition metals and metal oxides become one of the hottest topics in materials science due to their special properties and potential applications [1-3]. Amongst these materials, the supported and unsupported copper and copper oxide nanoparticles are of great interest due to their ad-

* Corresponding Author. E-mail: sayedbadawy@hotmail (S.M. Badawy)

vantages such as nontoxicity, abundance, high optical absorption coefficient and low band gap energies [4,5]. These characteristics make them prospective candidates for different applications such as catalysis, semiconductor equipment, solar/photovoltaic energy conversion, gas sensing, antimicrobial materials, luminescence sources field, emission devices, lithium-ion electrode materials and dye-sensitized solar cells [6-9]. Copper nanoparticles have a high antimicrobial activity against Bacillus Subtilis. Copper ions released may also interact with DNA molecules and intercalate with nucleic acid

bcrec_7984_2015 Copyright © 2015, BCREC, ISSN 1978-2993

Bulletin of Chemical Reaction Engineering & Catalysis, 10 (2), 2015, 170 strands. Copper ions inside bacterial cells also disrupt biochemical processes [10]. CuO is a p-type semiconductor with a narrow band gap (1.2 eV) and exhibits a number of interesting properties [11]. Copper oxide based materials have widespread applications [12, 14]. CuO crystal also has photocatalytic or photovoltaic properties and photoconductive functionalities [15]. As CuO is cheaper than silver, easily mixes with polymers and relatively stable in terms of both chemical and physical properties, it finds a wide application [16]. The synthesis of metallic copper nanoparticles surrounded by amorphous CuO, in the presence of poly(vinylpyrrolidone) as a protecting agent, via a polyol method in ambient atmosphere was described in previous works [17]. The novel synthesis of copper and copper oxide nanoparticles using the chemical reduction method and its physicochemical characterization were reported [18]. The nanoparticles have been prepared using copper(II) succinate as precursor. Copper nanoparticles are initially formed and subsequently oxidized to copper oxide. The copper nanoparticles showed excellent activity against Escherichia coli and Staphylococcus aureus, with excellent inhibition zones [18]. Copper based nano-material containing different phases of copper, CuO/Cu2O/Cu, was prepared by the glycine assisted combustion method [19]. The results of X-ray diffraction (XRD) and scanning electron micrographs (SEM) revealed that the investigated method led to formation of mixture of CuO/Cu 2O/Cu by using a certain amount of glycine as a fuel. CuO, Cu2O nanoparticles and Cu/Cu2O composite nanoparticles of different sizes have been hydrothermally synthesized by varying the reaction temperature and in the presence of biocompatible surfactants; polyoxyethylene, sorbitan laurate, polyethylene glycol 1000 and polyethylene glycol 8000 [20]. The coppercontaining phases - copper oxide (CuO), cuprous oxide (Cu 2O), copper aluminate (CuAl2O4), zinc oxide (ZnO) and zinc aluminate (ZnAl2O4) were prepared by thermal reactions [21]. Capture of CO2 and conversion to syn-gas by the samples of copper and zinc aluminates at higher temperatures were observed. In the present work, the synthesis of Cu nanoparticles was studied using a modified reducing method in aqueous medium. Cuprous oxide (Cu2O), which was later confirmed in XRD, may be produced via partial oxidation of Cu in aqueous or acid medium. Cu2O may be also formed by reduction of copper ions Cu 2+ to cuprous ions Cu2+. Then the cuprous ions react

with hydroxyl in the aqueous medium to form cuprous oxide. For synthesis of pure Cu, such a finding consider a non-aqueous system to avoid the formation of copper oxide. Further chemical and morphology structures were investigated for Cu/Cu2O nanoparticles. The catalytic activity of Cu/Cu2O nanoparticles for the decomposition of hydrogen peroxide, in comparison with manganese oxide MnO2, was investigated and analyzed by fitting various kinetic order equations. 2. Materials and Methods 2.1. Synthesis of Cu/Cu2O Nanoparticles Cu/Cu2O powder was obtained by reaction of an aqueous solution of copper sulfate pentahydrate (Fluka) with hydrazine hydrate (SigmaAldrich) in ammonia chloride solution. In a modification of preparation of copper powder [22], 100 ml solution containing 50 g (80%) hydrazine hydrate was added dropwise for 40 min to 200 ml aqueous mixture of CuSO4·5H2O (40g), NH4Cl (15 g) and aqueous ammonia (70 ml, 28%) with stirring. The temperature was kept below 30 °C. Then, the solution was heated to 80 °C for 2 h to carry out the reaction sufficiently, to reduce the copper ion in the solution to metallic copper. The Cu/Cu2O powder was recovered from the solution by filtration, washed and dried under vacuum. 2.2. Characterizations X-ray diffraction pattern was recorded in the continues scanning mode at room temperature on an EMPYREAN Diffractometer system operated at 45 kV and a current of 30 mA using Cu tube with Cu Kα radiation (λ = 1.5406 Å). The diffraction intensities were recorded from 10o to 80o, in 2θ angles. The diffraction intensity was compared with the standard ICSD collection files. Elemental analysis was performed using Energy Dispersive X-ray Fluorescence system (Jeol JSX - 3222 element analyzer) system. The scanning electron microscope for samples was performed using SEM (Quanta 250 Field Emission Gun), with accelerating voltage 30 kV and magnification 14X up to 1000000. The morphological analysis was analyzed using transmission electron microscopy (JEOL JEM2100). 2.3. Catalytic decomposition of hydrogen peroxide To investigate the catalytic activity of Cu/Cu2O nanoparticles for the decomposition of

Copyright © 2015, BCREC, ISSN 1978-2993

Bulletin of Chemical Reaction Engineering & Catalysis, 10 (2), 2015, 171 hydrogen peroxide (0.09 M H2O2), different Cu/Cu2O concentrations, 0.08, 0.20 and 0.40 g/l, at 25 ºC were used. The solution was stirred uniformly. After an interval time; 5ml of the reaction mixture was withdrawn by pipette from the beaker and was rapidly added to 5 ml of 1.0 M H2SO4 solutions and then titrated against 0.02 M of KMnO4 solution until color disappearance. 3. Results and discussion 3.1. Synthesis of Cu/Cu2O nanoparticles Hydrazine hydrate and NH4Cl/NH3·H2O were used as reductant and buffer agent, respectively [22]. Hydrazine (N2H4) is a powerfully strong reductant widely used in various chemical operations. The optimum reduction of Cu can be achieved at pH > 11 [23]. The solution of Cu2+ was blue before being reduced, and became yellow after reduction. In this process, the following chemical reaction occurred:

In aqueous ammonia media, ammonia reacts with Cu2+ according to the reaction (1) and [Cu(NH3)4]2+ complex was reduced to obtain fine copper powder as being seen in Equation (2). The copper ions Cu 2+ may be reduced to cuprous ions. Then the cuprous ions react with hydroxyl in the system to form cuprous oxide [24]:

Cuprous oxide may be produced via oxidation of Cu as follow:

Additives, such as: water and acids, affect the rate of this process as the further oxidation to copper(II) oxides [25]. 3.2. Characterizations The characterization techniques that are commonly used to study the crystal structure and chemical composition of products include X-ray diffraction and Energy dispersive X-ray fluorescence (EDXRF). Figure 1 showed the XRD pattern of the product prepared by the solution containing CuSO4·5H2O and hydrazine hydrate. The diffractogram exhibits the characteristic peaks of two phases; crystalline metallic copper (cubic) and Cu2O (cubic). This means that Cu2+ ions were reduced to Cu and Cu+1. The spectrum of Cu shows the peaks corresponding to 2θ = 43.23, 50.51, 74.30 with dspacing = 2.09, 1.81, 1.28, respectively. All peaks can be attributed to the cubic form of metallic copper [26]. The spectrum of Cu 2O shows the peaks corresponding to 2θ = 29.63, 36.37, 42.45, 61.64, 73.75 with d-spacing = 3.02, 2.46, 2.13, 1.51, 1.28, respectively. These peaks are

Figure 1. XRD of Cu/Cu2O nanoparticles Copyright © 2015, BCREC, ISSN 1978-2993

Bulletin of Chemical Reaction Engineering & Catalysis, 10 (2), 2015, 172 very close to that given by JCPDS data of XRD for copper (cubic) and Cu2O (cubic). No other diffraction peaks arising from metal CuO appear in the XRD patterns. Energy dispersive X-ray fluorescence (XRF) was carried out to determine elemental composition of nanoparticles. The spectrum (Figure 2) shows two peaks CuKα (8.06 keV) and CuKβ (8.93 keV) characteristic of copper with 97.25% element content. The impurities calculated from XRF are 2.75% element of sulfur. Figure 3 shows the TEM image of Cu/Cu2O nanoparticles synthesized by chemical reduction with hydrazine hydrate. It shows that higher tendency of agglomerations of nanoparticles in agglomerated bulks. On the edges, few particles are single crystals of face-centered cubic structures. The actual size of nanoparticles is estimated from TEM micrograph. The average particle size is about 11-14 nm. The morphology of the prepared particles was studied by SEM as shown in Figure 4.

Figure 2. XRF of Cu/Cu2O nanoparticles

Figure 3. TEM of Cu/Cu2O nanoparticles

From SEM photographs, we can distinctly find monodispersed and agglomerated particles of two micron sizes. The particles are sphericallike and have uniform sizes of about 18 μm and 0.80 μm (Figure 4). These results confirm the analysis by XRD for the formation of copper and cuprous oxide nanoparticles by chemical reduction with hydrazine hydrate. 3.3. Catalytic decomposition of H2O2 The decomposition of hydrogen peroxide (H2O2) has been used as a model reaction for the investigation of the catalytic activity of various metal complexes [27] as follow:

The rate of decomposition can be accelerated by transition metal compounds due to their higher activity. Manganese oxide is considered as an active catalyst for decomposition of hydrogen peroxide. The amount of the decomposed H2O2 % was estimated against the time of catalytic reaction using different Cu/Cu 2O concentrations, 0.08, 0.20 and 0.40 g/l, at room temperature as shown in Figure 5. The decomposition increases and then slows with reaction time. The decomposition of hydrogen peroxide can be described by the second order kinetic expression as follow:

The kinetic of the catalytic activity of Cu/Cu2O nanoparticles for the decomposition of hydrogen peroxide was analyzed by fitting various kinetic order equations. Figure (6) indicates that the decomposition of H2O2 on

Figure 4. SEM of Cu/Cu2O nanoparticles


Bulletin of Chemical Reaction Engineering & Catalysis, 10 (2), 2015, 173 Cu/Cu2O is in a second-order reaction with rate constants of 0.013, 0.076 and 0.145 M-1.min-1 for Cu/Cu2O concentrations of 0.08, 0.20 and 0.40 g/l, respectively. The catalytic effect of Cu/Cu2O was compared to that of manganese oxide for the decomposition of hydrogen peroxide at catalyst concentration of 0.08 g/l. Figure 7 shows that the reaction rate of Cu/Cu2O (0.013 M-1.min-1) is less than the reaction rate of MnO2 (0.26 M-1.min-1). The catalytic activity of hydrogen peroxide by Cu/Cu2O is less than the catalytic activity of MnO2 due to the presence of copper metal Cu with cuprous oxide Cu2O. The affinity of HO• towards the surfaces of the oxides, depends on the type of oxide. The obtained trend for adsorption energies of HO• onto the different metal oxides is inversely proportional to the variation in ionization potential of the metal cation [28].

4. Conclusion Copper/Copper oxide Cu/Cu2O nanoparticles were synthesized by the chemical reduction method using hydrazine as reducing agent and copper sulfate pentahydrate as precursor. Copper nanoparticles were initially formed and subsequently partially oxidized to copper oxide. Cu2O may be formed by reduction of copper ions Cu2+ to cuprous ions Cu2+. Then the cuprous ions react with hydroxyl in the aqueous medium to form cuprous oxide. For synthesis of pure Cu, unaqueous system is considered to avoid the formation of copper oxide. The XRD analysis revealed the pattern of the fcc crystal structure of copper Cu metal and cubic cuprites structure for copper oxide Cu2O. The SEM showed monodispersed and agglomerated particles with two micron sizes of about 180 nm and 800 nm, respectively. The TEM showed few single crystal particles of face-centered cubic structures with average particle size about 1114 nm. The second-order equation provides the best correlation for the catalytic decomposition of H2O2 on Cu/Cu2O. The catalytic activity of hydrogen peroxide by Cu/Cu2O is less than the catalytic activity of MnO2 due to the presence of copper metal Cu with cuprous oxide Cu2O. Acknowledgments Financial support from Aljouf University (Research Project Number 232/34) is gratefully acknowledged. References

Figure 5. Decomposition of H2O2 % (percentage of the reacted H2O2) against reaction time, min

[1]

Deraz, N.M., Alarifi, A. (2012). Novel processing and magnetic properties of hematite/maghemite nano-particles. Ceramics International 38: 4049-4055.

Figure 6. 1/(a-x) against time of reaction, min, for decomposition of H2O2 on Cu/Cu2O, where a and x are the initial and the reacted concentrations of H2O2, respectively.

Figure 7. Comparison between Cu/Cu2O and MnO2 for the decomposition of hydrogen peroxide, where a and x are the initial and the reacted concentrations of H2O2, respectively


Bulletin of Chemical Reaction Engineering & Catalysis, 10 (2), 2015, 174 [2]

Deraz, N.M. (2012). Magnetic behavior and physicochemical properties of Ni and NiO nano-particles. Current Applied Physics 12: 928-438.

[16]

Xu, J.F., Ji, W., Shen, Z.X., Tang, S.H., Ye, X.R., Jia, D.Z., Xin, X.Q. (1999). Preparation and characterization of CuO nanocrystals. J. Solid State Chem. 147: 516-519

[3]

Deraz, N.M. (2012). Formation and Magnetic Properties of Metallic Nickel Nano - Particles. Int. J. Electrochem. Sci. 7: 4608-4616.

[17]

[4]

Xu, S., Sun, D.D. (2009). Significant improvement of photocatalytic hydrogen generation rate over TiO2 with deposited CuO. Int. J. Hydrogen Energy 34:6096- 6104.

Park, B.K., Jeong, S., Kim D., Moon, J., Lim, S., Kim, J.S. (2007). Synthesis and size control of monodisperse copper nanoparticles by polyol method. Journal of Colloid and Interface Science 311: 417-424

[18]

Karthik, A., Geetha, K. (2013). Synthesis of Copper Precursor, Copper and its oxide Nanoparticles by Green Chemical Reduction Method and its Antimicrobial Activity. Journal of Applied Pharmaceutical Science 3 (05): 016-021.

[19]

Abd-Elkader, M., Deraz, N.M. (2013). Synthesis and Characterization of New Copper based Nanocomposite. Int. J. Electrochem. Sci., 8: 8614-8622.

[5]

Wu, N.L., Lee, M.S. (2004). Enhanced TiO2 photocatalysis by Cu in hydrogen production from aqueous methanol solution. Int. J. Hydrogen Energy 29: 1601-1605.

[6]

Weizhong, L., Zhongkuan, L., Hui, Y., Bo, L., Wenjiang, W., Jianhong, L. (2010). Effect of processing conditions on sonochemical synthesis of nanosized copper aluminate powders. Ultrasonics Sonochemistry 17: 344-351.

[20]

[7]

Choon-Hoong, T., Yanwu, Z., Xingyu, G., Andrew, W. Thye-Shen, S., Chorng-Haur, S. (2008). Field emission from hybrid CuO and CuCO3 nanosystems. Solid State Communication 145:241-245.

Giannousi, K., Avramidisb, I., DendrinouSamara, C. (2013). Synthesis, characterization and evaluation of copper based nanoparticles as agrochemicals against Phytophthora infestans. RSC Adv. 3: 21743-21752.

[21]

[8]

Chao, L., Wei, W., Shaoming, F., Huanxin, W., Yong, Z., Yanghai, G., Rongfeng, C. (2010). A novel CuO-nanotube/SnO2 composite as the anode material for lithium ion Batteries. Journal of Power Sources 195: 29392944.

Raskar, R.Y., Gaikwad, A.G. (2014). The Uses of Copper and Zinc Aluminates to Capture and Convert Carbon Dioxide to Syn-gas at Higher Temperature. Bulletin of Chemical Reaction Engineering & Catalysis, 9 (1): 1-15. (DOI: 10.9767/bcrec.9.1.4899.1-15)

[22]

[9]

Xue, W., Chenguo, H., Hong, L., Guojun, D., Xiaoshan, H., Yi, X. (2010). Synthesis of CuO nanostructures and their application for nonenzymatic glucose sensing. Sensors Actuator B 144: 220-222.

Songping, W., Shuyuan, M. (2006). Preparation of micron size copper powder with chemical reduction method. Materials Letters 60: 2438-2442

[23]

Rupareli, J.P., Chatterjee, A.K., Duttagupta S. P., Mukherji, S. (2008). Strain specificity in antimicrobial activity of silver and copper nanoparticles. Acta Biomaterialia 4: 707-771

Chen, J.P., Lim, L.L. (2002). Key factors in chemical reduction by hydrazine for recovery of precious metals. Chemosphere 49: 363-370

[24]

Musa, T., Akomolafe, M.J., Carter, S. (1998). Production of cuprous oxide, a solar cell material, by thermal oxidation and a study of its physical and electrical properties. Energ. Mater. Sol. C. 51: 305-316.

He, P., Shen, X., Gao, H. (2005). Sizecontrolled preparation of Cu2O octahedron nanocrystals and studies on their optical absorption. Journal of Colloid and Interface Science 284: 510-515.

[25]

Wayne, H. (2002). Copper compounds. Ullmann’s Encyclopedia of industrial chemistry, Wiley-VCH, Weinheim.

[12]

Macilwain, C. (2000). Bell labs win superconductivity patent. Nature 403: 121-122.

[26]

[13]

MacDonald, A.H. (2001). Copper oxides get charged up. Nature 414: 409-410.

Ingunta, R., Piazza, S., Sunseri, C. (2008). Novel procedure for the template synthesis of metal nanostructures. Electrochem. Commun., 10: 506-509

[14]

Lanza, F., Feduzi, R., Fuger, J. (1990). Effects of lithium oxide on the electrical properties of CuO at low temperatures. J. Mater. Res. 5: 1739-1744.

[27]

[15]

Kwak K., Kim, C. (2005). Viscosity and thermal conductivity of copper oxide nanofluid dispersed in ethylene glycol. Korea–Australia Rheo J. 17: 35-40

Skounas, S., Methenitis, C., Pneumatikakis, G., Morcellet, M. (2010). Kinetic Studies and Mechanism of Hydrogen Peroxide Catalytic Decomposition by Cu(II) Complexes with Polyelectrolytes Derived from L-Alanine and Glycylglycine. Bioinorganic Chemistry and Applications. 2010, ID 643120, 9 pages.

[10]

[11]
